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Vol.48, No.1, June 2015, pp.17-25
17
Low temperature synthesis of CaZrO3 nanoceramics from CaCl2–NaCl
molten eutectic salt
Rahman Fazli1*
and F. Golestani-Fard2
1. Young Researchers and Elite Club, Zanjan Branch, Islamic Azad University, Zanjan, Iran
2. School of Metallurgy and Materials Engineering, Iran University of Science and Technology, Tehran, Iran
Received: 13 Dec. 2014 ; Accepted: 6 May 2015
*Corresponding Author Email: [email protected], Tel: +98-937-2139453
Abstract
CaZrO3 nanoceramics were successfully synthesized at 700 C using the molten salt method, and the
effects of processing parameters, such as temperature, holding time, and amount of salt on the
crystallization of CaZrO3 were investigated. CaCl2, Na2CO3, and nano-ZrO2 were used as starting
materials. On heating, CaCl2–NaCl molten eutectic salt provided a liquid medium for the reaction of
CaCO3 and ZrO2 to form CaZrO3. The results demonstrated that CaZrO3 started to form at about 600C
and that, after the temperature was increased to 1,000C, the amounts of CaZrO3 in the resultant powders
increased with a concomitant decrease in CaCO3and ZrO2 contents. After washing with hot distilled
water, the samples heated for 3 h at 700C were single-phase CaZrO3 with 90–95 nm particle size.
Furthermore, the synthesized CaZrO3 particles retained the size and morphology of the ZrO2 powders
which indicated that a template mechanism dominated the formation of CaZrO3 by molten-salt method.
Keywords: calcium zirconate, molten salt method, nanomaterials, template growth.
1. Introduction
Calcium zirconate (CaZrO3) due to its valuable
properties, such as high melting point
(2,340C), high dielectric permittivity, and
low dissipation factor, is a ceramic material
that is currently being used in a wide range of
applications: multilayer ceramic capacitors,
solid electrolyte, crystalline host for
phosphorescence materials, moderate
temperature thermal barrier catalyst, and so on
[1–3]. There are several methods for the
synthesis of this material. CaZrO3 powders is
conventionally synthesized via a high
temperature (1500C) solid state reaction of
powdered calcium oxide (CaO) (or calcium
carbonate (CaCO3)) and zirconia (ZrO2)
(conventional mixed oxide synthesis (CMOS)).
As the reactions are generally controlled by
slow diffusion mechanisms, highly reactive
raw materials, high temperatures, and long
duration have to be used for the reactions to
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achieve completion. The resultant product is
a hard mass, which often needs to be crushed
and ground to achieve the desired particle size
[4]. Other methods such as electrofusion [5],
wet chemical [6–8], combustion [9], and
mechanical alloying (MA) [10] have been
reported for synthesis of calcium zirconate.
Almost all the aforementioned methods are not
commodious, because their synthesis
temperatures are high in solid state and
electrofusion methods and thus need so much
thermal energy and time. Therefore, it is
necessary to follow methods that decrease
synthesis temperature and time. Besides the
above techniques, a low temperature
synthesis technique called molten salt
synthesis (MSS), is beginning to attract
interest. In this method, a salt is used as a
liquid medium, therefore, the reactions are
faster and synthesis is complete in significantly
lower temperature and time [4, 11, 12]. Zushu
Li et al.’s investigation is perhaps the most
important research on the synthesis of CaZrO3
via molten salt method that prepared CaZrO3
powder at 1,050C for 5h [4]. In this work,
CaZrO3was synthesized by heating CaCO3,
sodium carbonate (Na2CO3), sodium chloride
(NaCl), and nano-ZrO2 mixture, and the effects
of temperature, holding time, and salt to oxide
ratio on synthesis process were investigated.
Also, synthesis mechanism was analyzed.
2. Experimental Procedure
2.1. Dispersion of nano-ZrO2
Nano-ZrO2 (Neutrino, Germany, D50 = 60
nm, > 99% pure), hydrochloric acid (HCl),
and distilled water (pH = 7.2) were used for
the dispersion of nano-ZrO2. First, pH of
distilled water was decreased to 4 using HCl
by gently adding it to distilled water and then
measuring the pH using pH meter (Jenway,
model 3540). After regulating the pH of
distilled water, agglomerated nano-ZrO2
particles were added and stirred for 1h using
electrical stirrer. Then, this suspension was
placed for 2min in an ultrasonic probe and
then stirred for 1h again. The process of
stirring and placing in ultrasonic probe were
alternatively repeated several times to obtain
extremely dispersed particles. Then, a little
amount of the stirring suspension was poured
on a hot glass lamella using a syringe.
Thereafter, water from the suspension was
rapidly vaporized, separated and dispersed
particles of nano-ZrO2 remained in the
container. The particle size of dispersed
nano-ZrO2 was determined via dynamic light
scattering (DLS, Malvern, ZEN 3600),
scanning electron microscopy (SEM, Tescan
Vega II), and transition electron microscopy
(TEM, CM 200, Philips).
2.2. Preparation of powder mixture
Na2CO3 (Merck, Germany, D50 = 1mm, 99.5%
pure), calcium chloride (CaCl2) (Merck,
Germany, D50 = 4 mm, 99.5% pure), and nano-
ZrO2 (Neutrino, Germany, D50 = 60 nm, > 99%
pure) were used as starting materials. First,
stoichiometric compositions of Na2CO3 and
CaCl2 were completely mixed and the obtained
dual mixture was heated at 150C for 12h to
dry. Then, this salt was added to completely
dispersed nano-ZrO2 solution and the final
suspension was stirred for 1 h to homogenize
extremely. The mixture was fully dried at
120C for 12h. Molar ratio of final mixture was
ZrO2:Na2CO3:CaCl2 = 1:1:1.4. Agglomerations
of obtained powder which was completely
homogenous were broken using an agate
mortar and then sifted to pass through a 325
mesh screen (45 µm). Finally, the mixture (20
g) was placed in an alumina crucible covered
with an alumina lid, heated to 600; 650; 700;
800; 900; and 1,000C and held for 1, 3, and
5h. For investigating the effect of salt to oxide
ratio on the synthesis process, the samples were
heated at optimum temperature with 1:1, 2:1,
3:1, and 4:1 salt to oxide ratios. The heating
and cooling rates were 3 C/min and 5 C/min,
respectively. After cooling to room
temperature, the solidified mass was washed
and filtered in hot distilled water five times to
remove the salts. Then, the obtained powder
was dried at 120 C for 4 h. The phase
formation, morphology, and elemental analysis
of the synthesized powders were characterized
via X-ray diffraction (XRD, Philips pw3710),
SEM (TescanVega II), and X-ray fluorescence
(XRF, Philips 2404), respectively.
3. Results and discussion
3.1. Dispersed nano-ZrO2
SEM micrograph of agglomerated nano-ZrO2
particles has been shown in Figure 1. It is
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obviously observed that particle size of
zirconia was in the range of 200–250 nm.
This issue can be attributed to adherence and
thereupon agglomeration of nano-ZrO2
particles.
Fig. 1. SEM micrograph of agglomerated nano-ZrO2
particles
SEM micrograph of dispersed nano-ZrO2
particles has been shown in Figure 2. As
seen, particle size of nano-ZrO2 was in the
range of 60–80 nm. This object was
confirmed by TEM micrograph of these
particles shown in Figure 3.
Fig. 2. SEM micrograph of dispersed nano-ZrO2
particles
Fig. 3. TEM micrograph of dispersed nano-ZrO2
particles
Figure 4 shows particle size distribution
curve of nano-ZrO2 suspension measured via
DLS method. It is seen that distribution of
particle size was centralized in the range of
60–70 nm which means that almost all
agglomerations were broken and nano-ZrO2
particles were successfully dispersed.
Fig. 4. Particle size distributing curve of nano-ZrO2
suspension
3.2. Thermogravimetric analysis (TGA) of
synthesis process
DTA/TG analysis was performed to determine
the proper reaction temperature range as well
as the reaction order in the molten salt method.
Figure 5 indicates DTA/TG curve of Na2CO3,
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CaCl2, and nano-ZrO2. The DTA curve
exhibits an endothermic peak (peak a), which
is associated with a slow weight loss (10%) in
the TG curve at 100C. This weight loss is
attributed to dehydration of the precursors.
The small endothermic peak at approximately
150C (peak b) is related to the reaction
between Na2CO3 and CaCl2. The big
endothermic peak at about 500C (peak c) is
attributed to melting of CaCl2–NaCl eutectic
salt. The exothermic peak at approximately
600C (peak d) which is associated with a
slow weight loss in the TG curve is related to
formation of CaZrO3. The small exothermic
peak at 700C (peak e) is interpreted as the
crystallization of the CaZrO3 phase.
Fig. 5. DTA/TG curve of CaCl2, Na2CO3, and nano-
ZrO2 mixture
3.3. Effect of temperature
Figure 6 shows XRD patterns of the samples
heated for 3h at different temperatures. As
obviously observed, optimum temperature for
these samples was 700C. At this
temperature, the samples were single-phase
CaZrO3 and CaCO3 and ZrO2 peaks were not
observed. In other words, ZrO2 and CaCO3 were
completely transformed to CaZrO3. At
temperatures above 700C, the samples were
likewise single-phase CaZrO3 and just their
crystallinity was increased. This object was
confirmed by means of increase in peak’s
intensity. At 1,000C, the peak’s intensity
were insignificantly decreased and partly
become wider that can be attributed to acceding
decomposition temperature of CaZrO3. Thus,
increase in temperature was a very effective
factor for completion of synthesis process.
Fig. 6. XRD patterns of the samples (water washed)
heated for 3 h at different temperatures
Energy dispersive X-ray spectroscopy
(EDS) micrograph of the samples heated at
700C for 3h shown in Figure 7 confirmed
that optimum temperature for synthesized
samples was700C. As seen, almost only [Ca],
[Zr], and [O] elements were observed and
other elements were eliminated.
Fig. 7. EDS micrograph of the samples heated at 700C for 3h
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3.4. Effect of holding time
Figure 8 provides XRD patterns of the
samples heated for different holding times at
700C. As observed, optimum holding time
for these samples was 3 h. In this holding
time, synthesis process was complete and the
samples were single-phase CaZrO3. Also,
CaCO3 and ZrO2 peaks were not observed. In
1h holding time, CaCO3 and ZrO2 peaks were
seen, in addition to CaZrO3 peaks. In other
words, synthesis process was not completed.
In 5 h holding time, the samples were
likewise single-phase CaZrO3 and just
intensity of their peaks was insignificantly
increased compared with 3h holding time,
which means that their crystallinity was
venially increased. Thus, increase in holding
time, before optimum holding time, was an
effective factor for completion of synthesis
process and after this holding time did not
have a significant effect.
Fig. 8. XRD patterns of the samples (water washed)
heated at 700C with different holding times
3.5. Effect of salt amount
XRD patterns of the samples heated with
different salt to oxide ratios at 700C have
been shown in Figure 9. It resulted in an
optimum salt to oxide ratio of 2:1, as the
synthesis process was completed in this
ratio. In salt to oxide ratio of 1:1, the
samples still did not become single-phase
CaZrO3, and it was necessary to increase the
salt to oxide ratio for completion of the
synthesis. With increase in the salt to oxide
ratio of 2:1 to higher values, the samples
remained single-phase and during more
increase in salt to oxide ratio, more increase in
peaks intensity and thereupon more increase in
crystallinity property were seen. Thus,
increase in salt to oxide ratio was a very
effective factor for the completion of
synthesis process.
Fig. 9. XRD patterns of the samples (water washed)
heated at 700 C for 3 h with different salt to oxide
ratios
3.6. Particle size
Figure 10 shows SEM micrographs of the
samples synthesized at different temperatures.
As seen, the particle size of CaZrO3
synthesized at 700, 800, and 900C was in the
range of 90–95 nm. Whereas, the particle size
of CaZrO3 synthesized at 1,000C was in the
range of 180–200 nm which can be attributed
to grain growth phenomenon started at above
1,000C.
Particle size distribution curve of CaZrO3
particles synthesized at 700C for 3h
measured via DLS method has been shown in
Figure 11. As seen, distribution of particle
size was centralized in the range of 90–95
nm.
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Fig. 10. SEM micrographs of the samples synthesized for 3 h at (a) 700C; (b) 800C; (c) 900C; (d) 1,000C
Fig. 11. Particle size distribution curve of CaZrO3 particles synthesized at 700C for 3h
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3.7. CaZrO3 synthesis mechanism
NaCl, CaCl2, or NaCl–CaCl2 salts could be
used as molten salt media. According to
Figure 12 [13], as melting point of eutectic salt
(504C) was lower than both singular CaCl2
(771C) and NaCl (801C) salts, NaCl–
Na2CO3 eutectic salt was more suitable.
Fig. 12. CaCl2 –NaCl phase diagram [14]
On heating the mixture, the first reaction
was between Na2CO3 and CaCl2 (Reaction 1).
2 2 3 3
0
2
118123 198
CaCl Na CO CaCO NaCl
G T
(1)
This is consistent with the thermodynamic
prediction that reaction 1 could occur at as low
as room temperature, because the ∆G0 is
negative in the whole temperature range
between 25 and 600C [14]. Once Reaction
(1) was completed, Na2CO3 would disappear,
and the salt assembly would become one that
is essentially composed of NaCl and excess
CaCl2. The molar ratio between NaCl and the
excess of CaCl2 is 2:0.4, and the NaCl–CaCl2
phase diagram indicates that salt with such a
composition will start to melt at 504C
(eutectic temperature) in the areas where the
eutectic exists and become completely liquid
at about 650C (liquidus temperature).
This molten NaCl–CaCl2 salt provided a
reaction medium for the CaZrO3 synthesis
and also acted as a very proper catalyzer. Thus,
Reaction 2 started at about 600C that was
very lower than its thermodynamic prediction
(670C) [14]. With increase in the
temperature to 600C, CaCO3 reacted with
ZrO2 and some CaZrO3 was formed. With
increase in the temperature to 650C, NaCl–
CaCl2 salt completely melted, and reaction 2
became very more complete and rapid. Due
to very high reactivity of nano size ZrO2,
synthesis of CaZrO3 was completed at 700C.
3 2 3 2 0
193400 289
CaCO ZrO CaZrO CO
G T
(2)
To understand the reaction mechanisms,
the whole synthesis process of CaZrO3
discussed above has schematically been
illustrated in Figure 13.
Two main mechanisms, “template-growth”
and “dissolution-precipitation,” were involved in
MSS. Solubility of reactants in the molten salt
plays an important role in MSS. This not only
affects the reaction rate but also the
morphologies of the synthesized particles. If
both of the reactants are soluble in the molten
salt, then the product phase will be readily
synthesized via precipitation from the salt
containing the dissolved reactants
(dissolution–precipitation mechanism). In this
case the morphologies of the product grains
will generally be different from those of the
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reactants. However, if one of the reactants is
much more soluble than another, the more
soluble reactant will dissolve into the salt firstly
and then diffuse onto the surfaces of the less
soluble reactant and react in situ to form the
product phase. In this case, the morphology of
the synthesized grain will retain the less soluble
reactant (template-growth mechanism) [15, 16].
Fig. 13. Schematic diagram illustrating the synthesis of CaZrO3 powder by
heating nano ZrO2, CaCl2, and Na2CO3
According to some studies [17, 18],
CaCO3 is soluble in a chloride molten salt. Its
solubility in a NaCl-based salt at 700–1,000C
are on the order of 10−3
(molar fraction),
which is thousand times higher than that of
ZrO2 (on the order of 10−6
). Therefore, during
the MSS process, CaCO3would be dissolved
more in the NaCl–CaCl2 molten salt and react
with ZrO2 templates to form in situ CaZrO3.
This explains the similarity between the grain
shapes of the synthesized CaZrO3 and original
ZrO2 powder. The morphology and particle size
of the synthesized CaZrO3 grains was similar to
ZrO2 grains which mean that the “template-
growth” mechanism played a dominant role
in the low-temperature molten salt synthesis
of CaZrO3 nanoparticles (Fig. 14).
The chemical composition of product
powders determined via XRF analysis has
been shown in Table 1. As seen, after
washing, only minor contents of salt and other
contaminations remained in the synthesized
CaZrO3 powders. The main objective of this
table is to illustrate the feasibility of the
molten salt method for the synthesis of very
pure ceramic powders.
Table 1. Chemical composition of synthesized CaZrO3 in different reaction conditions
Weight Percent Reaction Condition
Al C Cl Si O Zr Ca Salt to oxide ratio Time (h) Temperature (oC)
0.01 0.03 0.08 0.14 59.92 19.89 19.93 2:1 3 600
0.01 0.02 0.08 0.12 59.93 19.90 19.94 2:1 3 650
0.02 0.01 0.07 0.13 59.93 19.91 19.93 2:1 3 700
0.01 0.01 0.08 0.11 59.92 19.92 19.95 2:1 3 800
0.02 0.02 0.07 0.12 59.91 19.92 19.94 2:1 3 900
0.02 0.03 0.06 0.12 59.91 19.91 19.95 2:1 3 1000
0.01 0.03 0.08 0.11 59.92 19.91 19.94 2:1 1 700
0.01 0.02 0.07 0.11 59.90 19.93 19.96 2:1 5 700
0.01 0.01 0.08 0.12 59.91 19.92 19.95 1:1 3 700
0.01 0.01 0.07 0.12 59.92 19.91 19.96 3:1 3 700
0.01 0.01 0.07 0.13 59.92 19.90 19.96 4:1 3 700
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4. Conclusions 1. Nano-size calcium zirconate powders
were synthesized via molten salt method.
Na2CO3, CaCl2, and nano- ZrO2 were used as
starting materials.
2. Optimum temperature for samples was
700C that was significantly lower than that
required by solid state method. Increase in
temperature was a very effective factor for
completion of synthesis process.
3. Optimum holding time for samples was
3h.Increase in holding time significantly did
not affect synthesis process.
4. Optimum salt to oxide ratio for samples
was 2:1. Increase in salt to oxide ratio resulted
in increase in the crystallinity property. Also,
increase in salt to oxide ratio was an effective
factor for completion of synthesis process.
5. Particle size of synthesized CaZrO3 was
90–95 nm. At above 1,000C, grain growth
phenomenon caused increase of particle size.
6. Similarity of morphology and particle
size of synthesized CaZrO3 to ZrO2 grains
showed that “template–growth” was dominant
mechanism in synthesis process.
7. Very minor contaminations components
remained in the synthesized powders indicated
that very pure CaZrO3nanoceramicswas
formed from CaCl2–NaCl molten eutectic salt.
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